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# Consider the oxidation of nitric oxide to nitrogen dioxide at 700 K: 1 NO + 502 : N02 KG :0 Suppose we start with a mixture of 1 mole of NO and 0.5...

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Consider the oxidation of nitric oxide to nitrogen dioxide at 700 K: NO + 1 2 O2 NO2 Ka = 2.0 Suppose we start with a mixture of 1 mole of NO and 0.5 mole of O2 in a vessel held at a constant pressure of 250 bar

5. Consider the oxidation of nitric oxide to nitrogen dioxide at 700 K:
1
NO + 502 : N02 KG : 2.0 Suppose we start with a mixture of 1 mole of NO and 0.5 mole of 02 in a vessel held at a
constant pressure of 250 bar. (a) Compute the equilibrium extent of reaction X and mole fraction of N02 assuming the
mixture behaves ideally. (You will have to solve an implicit equation for X.) Ans. X = 0.882 and yNo2 = 0.833. (b) At 250 bar, there are vapor-phase nonidealities. The following data on the fugacity
coefﬁcients 4%; are available at 700 K and 250 bar for various mixture compositions: SUNO 2902 yNOz GENO €502 923N02
0.00 0.00 1.00 1.19 1.10 0.989 0.10 0.05 0.85 1.16 1.08 0.991
0.20 0.10 0.70 1.14 1.07 0.996
0.30 0.15 0.55 1.12 1.06 1.000
0.40 0.20 0.40 1.10 1.06 1.020
0.50 0.25 0.25 1.09 1.06 1.030
0.60 0.30 0.10 1.08 1.06 1.050
0.67 0.33 0.00 1.08 1.07 1.060 (Note that for each mixture in the table, yNo : 2y02 .) Find the equilibrium extent of
reaction X and mole fraction of N02 accounting for nonidealities. Ans. X = 0.876 and yNo2 = 0.825.

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